Chemical Bonds and Properties

1. Describe the octet rule in terms of noble-gas configurations and stability.
2. Discuss the reasons behind metals being electropositive and non-metals being electronegative. (Cantab Exercise Question)
   1. Compare the formation of cations and anions.
   2. Why do metals tend to be electropositive while non-metals tend to be electronegative?
   3. State the number of electrons that must be lost by atoms of each of the following to achieve a stable electronic configuration.
3. Define chemical bond, also name its types.
4. How is an ionic bond formed? Explain with an example.
   Describe the formation of Na⁺ and Mg²⁺ cations.
   1. Describe the formation of cations for the following metal atoms.
   2. Represent the formation of cations for the following metal atoms using electron dot structures.
5. Describe the formation of anions for the following non-metal atoms:
   (a) Oxygen (atomic no. 8)
   (b) Fluorine (atomic no. 9)
   1. Describe the formation of anions by the following non-metals:
      (a) Sulphur (atomic number 16)
      (b) Chlorine (atomic number 17)
   2. Represent the formation of anions by the following non-metals using electron dot structures:
      (a) N
      (b) P
      (c) Br
      (d) H
6. For each of the following pairs of atoms, use electron dot and electron cross structures to write the equation for the formation of an ionic compound:
   a) Na and Cl
   b) Mg and F
7. For each of the following pairs of atoms, use electron dot and cross structures to write the equation for the formation of an ionic compound:
   (a) Mg and O
   (b) Al and Cl
8. Recognize the following compounds as having ionic bonds:
   a) MgO
   b) NaF
9. Write down a few properties of ionic bonds.
   1. Why do ionic substances have high melting points?
   2. Why do ionic substances conduct electricity?
   3. Why do ionic substances not conduct electricity as solids?
   4. Which of the following are likely to be ionic: CO₂, PH₁, Fe₂O₃, CH₄O, SiO₂, MgBr₂?
10. Define covalent bond. Discuss its properties in detail.
11. Draw electron cross and dot structures for:
    (a) CH₄, a major component of natural gas.
    (b) H₂O, which covers about 80% of the Earth's crust.
12. Draw electron cross and dot structures for the following molecules:
    a) CS₂, an organic solvent that dissolves sulfur, phosphorus, etc.
    b) N₂, a component of air.
    c) C₂H₄, ethene, a component of natural gas.
13. Explain the coordinate covalent bond in detail.
14. Distinguish and differentiate between non-polar covalent bonds and polar covalent bonds.
15. What is the difference between an electrovalent bond (ionic bond), a covalent bond, and a coordinate covalent bond?
    1. Differentiate between polar and non-polar covalent bonds.
    2. How is a coordinate covalent bond different from a normal covalent bond?
16. Discuss in detail the concept of intermolecular forces, including dipole-dipole forces and hydrogen bonding.
17. Discuss the nature of bonding, structure, and properties of a substance.
18. Discuss the conduction of electricity in ionic compounds.
19. Discuss the conduction of electricity through acids in detail.
20. Discuss how intermolecular forces influence melting and boiling points.
21. Discuss graphite and its uses in detail.
22. Discuss diamond, its structure, properties, and uses.
23. Discuss contrasting ionic and covalent compounds and their uses.
24. Define metallic bond. Also, explain the electron sea theory.
25. Write down the structure and properties of metals that make them suitable for industrial purposes.